Air contains 20% `O_(2)` by volume. How much volume of air will be required for the oxidation of 100 cc of acetylene

Options

A. 500 cc
B. 1064 cc
C. 212.8 cc
D. 1250 cc

Explanation

To solve the problem of how much volume of air is required for the oxidation of 100 cc of acetylene (C₂H₂), we can follow these steps:

### Step 1: Write the balanced chemical equation for the oxidation of acetylene.
The oxidation of acetylene produces carbon dioxide (CO₂) and water (H₂O). The balanced equation is:

\[ 2 \, \text{C}_2\text{H}_2 + 5 \, \text{O}_2 \rightarrow 4 \, \text{CO}_2 + 2 \, \text{H}_2\text{O} \]

### Step 2: Determine the volume of oxygen required for the oxidation of 100 cc of acetylene.
From the balanced equation, we see that 2 moles of C₂H₂ react with 5 moles of O₂. Therefore, the ratio of C₂H₂ to O₂ is:

\[ \frac{5 \, \text{O}_2}{2 \, \text{C}_2\text{H}_2} = \frac{5}{2} \]

If we have 100 cc of C₂H₂, we can calculate the volume of O₂ needed:

\[ \text{Volume of O}_2 = 100 \, \text{cc} \times \frac{5}{2} = 250 \, \text{cc} \]

### Step 3: Calculate the volume of air required to provide the necessary oxygen.
Since air contains 20% O₂ by volume, we need to find out how much volume of air is required to obtain 250 cc of O₂.

Let \( V \) be the volume of air required. Since 20% of this volume is O₂, we can set up the equation:

\[ 0.20 \times V = 250 \, \text{cc} \]

To find \( V \):

\[ V = \frac{250 \, \text{cc}}{0.20} = 1250 \, \text{cc} \]

### Conclusion
The volume of air required for the oxidation of 100 cc of acetylene is **1250 cc**.

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